Calorimetry Lab

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Introduction Calorimetry can be defined as the science used to determine changes in an energy system based on heat exchanges with the surroundings (Kotz 201). These types of experiments have numerous applications such as determining heat of reaction, dissolution or fusion for a specific solution or determining specific heat for certain metals. To do this, scientists use a device that is known as a calorimeter, which measures heat transferred to or from an object (Beran 287). Calorimetry is an important science that has innumerable applications. Drug companies use calorimetry to study the physical and energetic properties of substances to help create stable medical products (Clas 311). Dr. Randy Larsen, a research scientist at the University…show more content…
To dilute 50.0 mL of 3M HCl to 1M HCl, one must add 100.0 mL of deionized water. The same procedure would be used to dilute 3M NaOH to 1M NaOH. For this experiment, the objective is to find the enthalpy of neutralization for the reaction . Once the coffee cup calorimeter was assembled and the solutions properly diluted, 50.0 mL of each solution was measured into two separate, clean graduated cylinders. The temperatures of both the acid and base solutions were measured and recorded in degrees Celsius. The NaOH (base) solution was added to the calorimeter chamber first, then the acid was quickly added and the calorimetry lid was placed on the cup. The solution was continuously stirred throughout the experiment to keep the solution agitated and the reaction going. The temperature was read and recorded after the first thirty seconds, then at one minute, then every minute thereafter until six minutes had passed since the addition of the acid. This process was completed three separate times using the Styrofoam calorimeter. After the trials with the coffee cup calorimeter were complete, the trials with the market brand calorimeter began. For each trial, 50.0 mL of each solution was measured into two separate, clean graduated cylinders. The temperatures of both the acid and base solutions were measured and recorded. The NaOH (base) solution was added to the calorimeter…show more content…
In this reaction, more O-H bonds are forming to create water molecules and that energy is being released into the surroundings. During this reaction, the energy of the reactants would be greater than the energy of the products so the enthalpy (ΔH) would be a negative value (See Figure 1). During the trials using the coffee cup calorimeter, the results indicated that one of the tests was endothermic and showed a positive value for ΔH. The second trial indicated that there was no change in the system and the third trial showed that an exothermic reaction took place. When running the trials using the market brand calorimeter, all three trials indicated that an exothermic reaction had taken place. Based upon these findings, the market brand calorimeter produced more consistent and reliable results. When analyzing the results in Table 3, it is easy to see that the calorimeter was inconsistent. It produced different results each trial, despite the fact that the same solution was used in each reaction. In one of the trials, the testing indicated that there was no change in temperature at all, which is highly unlikely. In contrast, the market brand calorimeter produced consistent results, each trial indicating that an exothermic reaction had taken place (Table 4). When constructing a Styrofoam calorimeter, there are so many variables
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